Understanding how organic molecules can act as acids or bases and how this affects their reactivity.
Acids and Bases: Understanding the concept of acid and bases, their properties and definitions.
pH and pKa: Understanding the relationship between acidity, pH, and pKa values.
Acid-Base Equilibria: Understanding the equilibrium between weak acids and their conjugate bases.
Bronsted-Lowry Acid-Base Theory: Understanding the theory that explains how an acid donates a proton and how a base accepts a proton.
Lewis Acid-Base Theory: Understanding the theory that explains how a Lewis Acid accepts an electron pair and how a Lewis Base donates an electron pair.
Acid-Base Properties of Amino Acids: Understanding the role of amino acids in biochemistry, their acid-base properties and how they contribute to protein structure.
Acid-Base Titration: Understanding the process of determining the concentration of an acid or base solution by titrating with a known standard solution.
Buffer Solutions: Understanding how buffers work and their importance in controlling pH changes in biological and chemical systems.
Acid-Base Catalysis: Understanding the role of acid-base catalysis in organic reactions, in which an acid or a base is used to catalyze a reaction.
Acid-Base Indicators: Understanding the use of indicators to determine the pH of a solution and how they work.
Acid-Base Extraction: Understanding the process of separating acidic and basic compounds from a mixture by exploiting their differences in solubility.
Acid-Base Strength: Understanding the concepts of strong and weak acids and bases, as well as their relative strengths.
Acid-Base Reactions: Understanding the general reaction mechanism for acid-base reactions and their importance in organic chemistry.
Acid-Base Equations: Understanding the equations for acid-base reactions, including acid-base dissociation, proton transfer and neutralization reactions.
Acid-Base Balance in the Body: Understanding how the body maintains acid-base balance and the consequences of imbalances such as acidosis and alkalosis.
Strong acids: These are acids that completely dissociate in water to form hydrogen ions (H+).
Weak acids: These are acids that only partially dissociate in water to form hydrogen ions (H+).
Strong bases: These are bases that completely dissociate in water to form hydroxide ions (OH-).
Weak bases: These are bases that only partially dissociate in water to form hydroxide ions (OH-).
Lewis acids: These are electron pair acceptors that can form a covalent bond with a Lewis base.
Lewis bases: These are electron pair donors that can form a covalent bond with a Lewis acid.
Bronsted-Lowry acids: These are proton (H+) donors.
Bronsted-Lowry bases: These are proton (H+) acceptors.
Conjugate acids: These are species that are formed when a base accepts a proton. These are the product of the Bronsted-Lowry acid-base reaction.
Conjugate bases: These are species that are formed when an acid donates a proton. These are the product of the Bronsted-Lowry acid-base reaction.
Amphoteric molecules: These are molecules that can act as both an acid and a base, depending on the reaction conditions.
Neutral molecules: These are molecules that do not possess any acidic or basic properties.